Directions CHCЬ CH3CI CCla Write number of valence electrons for cach atom and find the total number of valence electrons Determine center atom and draw the skeleton Write the full Lewis Structure with all valence electrons Determine non-zero formal charges Center atom has regions Name the electronic geometry Center atom: # bonding atoms? # lone pairs? Name the molecular gcometry Draw the molecular geometry Identify polar covalent pairs. & Add dipole arrows for each polar bond Is there a net dipole? Is the molecule Polar or Nonpolar?

Directions CHCЬ CH3CI CCla Write number of valence electrons for cach atom and find the total number of valence electrons Determine center atom and draw the skeleton Write the full Lewis Structure with all valence electrons Determine non-zero formal charges Center atom has regions Name the electronic geometry Center atom: # bonding atoms? # lone pairs? Name the molecular gcometry Draw the molecular geometry Identify polar covalent pairs. & Add dipole arrows for each polar bond Is there a net dipole? Is the molecule Polar or Nonpolar?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter4: Molecular Structure And Orbitals

Section: Chapter Questions

Problem 123CP: Carbon monoxide (CO) forms bonds to a variety of metals and metal ions. liS ability to bond to iron...

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The atoms in a single bond can rotate about the internuclear axis without breaking the bond. The atoms in a double and triple bond cannot rotate about the internuclear axis unless the bond is broken. Why?
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(a) If these three balloons are all the same size, what angleis formed between the red one and the green one? (b) If additionalair is added to the blue balloon so that it gets larger,will the angle between the red and green balloons increase,decrease, or stay the same? (c) Which of the following aspectsof the VSEPR model is illustrated by part (b): (i) Theelectron-domain geometry for four electron domains is tetrahedral.(ii) The electron domains for nonbonding pairs arelarger than those for bonding pairs. (iii) The hybridizationthat corresponds to a trigonal planar electron-domain geometryis sp2.
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The VSEPR model was developed before any xenon com-pounds had been prepared. Thus, these compounds provided anexcellent test of the model’s predictive power. What would youhave predicted for the shapes of XeF₂, XeF₄, and XeF₆?
Consider the molecule PF4Cl. (a) Draw a Lewis structure forthe molecule, and predict its electron-domain geometry.(b) Which would you expect to take up more space, a P¬Fbond or a P¬Cl bond? Explain. (c) Predict the molecular geometryof PF4Cl. How did your answer for part (b) influenceyour answer here in part (c)? (d) Would you expect the moleculeto distort from its ideal electron-domain geometry? Ifso, how would it distort?
The compound SF3N has been synthesized.(a) Draw the Lewis diagram of this molecule, supposingthat the three fluoride atoms and the nitrogen atomsurround the sulfur atom. Indicate the formal charges.Repeat, but assume that the three fluorine atoms andthe sulfur atom surround the nitrogen atom.(b) From the results in part (a), speculate about whicharrangement is more likely to correspond to the actualmolecular structure.
A benzene molecule can be modeled as six carbon atoms arrangedin a regular hexagon in a plane. At each carbon atom, one of threeradicals NH2, COOH, or OH can be attached. How many suchcompounds are possible? (Make no distinction between single anddouble bonds between the atoms.)
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The structure of borazine, B3N3H6, is a six-membered ringof alternating B and N atoms. There is one H atom bondedto each B and to each N atom. The molecule is planar.(a) Write a Lewis structure for borazine in which the formalcharge on every atom is zero. (b) Write a Lewis structurefor borazine in which the octet rule is satisfied forevery atom. (c) What are the formal charges on the atomsin the Lewis structure from part (b)? Given the electronegativitiesof B and N, do the formal charges seem favorableor unfavorable? (d) Do either of the Lewis structuresin parts (a) and (b) have multiple resonance structures?(e) What are the hybridizations at the B and N atoms inthe Lewis structures from parts (a) and (b)? Would you expectthe molecule to be planar for both Lewis structures?(f) The six B—N bonds in the borazine molecule are allidentical in length at 1.44 Å. Typical values for the bondlengths of B¬N single and double bonds are 1.51 Å and1.31 A°, respectively. Does the value of the B—N…